In the following Bronsted acid/base reaction, identify the acid, base, conjugate acid, conjugate base.
HPO4^2- + OH- -> PO4^3- +H2O
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consider the following acids and their dissociation constants: HPO4^2-(aq)+H2O(l)<__->H3O^+(aq)+PO4^3-(aq). Ka=2.2x10^-13. HCOOH(aq)+H2O(l)<__->H3O^+(aq)+HCOO^-(aq). Ka=1.8x10^-4. a)which is the weaker acid, HPO4^2- or HCOOH? b)what is the conjugate base of HPO4^2-? c)which acid has the weaker conjugate base? d)which acid has the stronger conjugate base? e)which acid produces more ions?
1.Write the formula of the conjugate base for each of the following:a. HClO4 ______b. C6H5NH3+ ______c. HC4H7O2 ______d. H3PO42. Write the formula of the conjugate acid for each of the following:a. CO3-2 ______b. H2O ______c. H2PO4- ______d. SO3-2 ______3.The species HPO4-2is amphoteric. Write the 2 reactions showing this behavior of HPO4-2in aqueous solution.4. In the reactions below, identify the Bronsted Lowry acid, base, conjugate acid and conjugate base. H2S + NH3 ? HS- + NH4+HSO4- + OH- ? SO4-2 + H2OCO3-2 + H2O ? HCO3- + OH-
a) identify the conjugate acid-base pairs for the following reaction: H2O (aq) + CN- (aq)--->HCN (aq)+OH- (aq) b) give the conjugate acid of HSO4- and PO4 -2 c) give the conjugate base of HCLO4 and H3O+